What is at the difference between light and dark silicate minerals? Dark silicates are rich in iron and/or magnesium and are comparatively low in silica, Light silicates contain greater amounts of potassium, sodium, and calcium. 6. What is the second most common mineral in the crust? Quartz 7.
Redox Arena Lab Observations of Reagents for all lab parts Boiling chips- small white chalky chips with slight acidic smell Desiccant – large white chalky chips with chlorine like smell Acetic acid solution- clear liquid, no smell Granular zinc – silver, tiny chips Iodine chips - small sparkling silver chips Zinc ion and iodine-iodide-triiodide ion in water- brown liquid, strong smell Solid zinc iodide – white tiny chalk like solid Mineral oil – clear thicker liquid Silver nitrate (AgNO3) – clear liquid Magnesium turnings - Sodium thiosulfate- clear solution PART 1: Getting the Reactants Changes and Tests The zinc we weighed and added to the reactants (R) boiling tube was 1.99 grams. We also weighed 1.99 grams of iodine crystals and added them to the same tube. We then poured 0.17 M acetic acid to the R boiling tube and swirled it for about 1 min and 30 seconds before steam began to form and the solution turned brown. At this time we pipetted some of our mixture into another tube labeled “color solution tube (C)”. The solution was dark reddish brown.
Alkali Metals- Group 1 (IA) The alkali metals make up Group 1 of the periodic table. This family consists of the elements lithium, sodium, potassium, rubidium, cesium, and francium (Li, Na, K, Rb, Cs, and Fr, respectively). Group one elements share common characteristics. They are all soft, silver metals. Due to their low ionization energy, these metals have low melting points and are highly reactive.
Therefore compounds H2O, cyclohexane, C, and D are molecular compounds. Later testing the solubility of the compounds the lab results were the following. Solubility in water: compound A dissolved partially, compounds B and D dissolved nearly none, while compounds C and E dissolved freely in water. Solubility of the compounds in cyclohexane were: H2O nearly non dissolved so it formed layers of the two compounds, compounds A, B and C nearly non dissolved, while compound C partially dissolved, and compound D freely dissolved in cyclohexane. Finally arranging the compounds in order of increasing melting points are: Compound C with 187.06 °C, followed by compound D with 195.31, and Compound A, B and
The pure metal is very soft and can be easily formed and molded. The metal is pretty stable in air and does not become oxidized as fast as some of the other rare earth metals. Natural Erbium has all of six stable isotopes. There are also 9 radioactive isotopes of erbium such as erbium 169. Erbium 169 is an isotope used to treat rheumatoid arthritis and hemophilic arthropathies.
It is a weak bond, but is decisive in controlling the structure of both water and ice. In a water molecule, two hydrogen atom are bonded to an oxygen atom share a pair of electrons between them by a covalent bond. In H2O, only two of the six outer-shell electrons of oxygen are used for this purpose, leaving four electrons which are organized into two non-bonding pairs. Salts are ionic compounds that result from the neutralisation reaction of an acid and an alkali. They are composed of an equal number of cations and anions so that the product is electrically neutral.
Before it was heated, it was a shiny silver strip. It was smooth, malleable, and flat. When heated, a bright light was emitted. The new substance magnesium oxide was white, chalky, brittle, and dull. The light given off and the new substance formed both indicate a chemical change.
AP* Chemistry Solubility Equilibrium SOLUBILITY EQUILIBRIA (The Solubiliy-Product Constant, Ksp) We’ve got good news and we’ve got bad news… The good news: Solubility equilibrium is really simple. The bad news: You know all those solubility rules that state a substance is insoluble? They are actually a bit soluble after all. Only the future attorneys among you read the fine print. Soluble is often defined as greater than 3 grams dissolving in 100 mL of water.
Title Page Experiment Title: Experiment 4: Qualitative Analysis of Cations III – Mg2+, Ca2+, Fe3+, Ba2+. Aim To determine the presence of the cation II , Mn2+, Ni2+, Fe3+, (Fe2+), Al3+, Zn2+ by using separation method to confirm the presence of cation II in the test solution. Procedure Please refer to the laboratory manual page 30-31. Results Procedure Number and Ion | Test Reagent or Technique | Evidence of Chemical Change | Chemical(s) Responsible for Observation | Equation(s) for Observed Reaction | 1 | Centrifuge the solution. | A brown precipitate was formed.
Si, P, S and Cl are increasingly electronegative. They cannot form oxide ions from oxygen at all, so they behave as acids. The trend is from strongly basic oxides on the left-hand side to strongly acidic ones on the right, via an amphoteric oxide (aluminium oxide) in the middle. In addition, when going across the period 3 the acid-base nature of the oxides change from base to amphoteric and finally to become acid. This is because the less electronegative sodium has a weak Na-O bond and the oxygen is more easily given up to reacts with H+.